SOL Review 6 Stoichiometry. Consider: 4NH 3 + 5O 2  6H 2 O + 4NO Many conversion factors exist: 4 NH 3 6 H 2 04NO 5O 2 (and others) 5 O 2 4 NO4 NH 3.

Slides:

Advertisements

Similar presentations

Stoichiometric Calculations

Advertisements

Stoichiometry (Yay!).

Limiting Reactants & Percent Yield. Limiting Reactants  The reactant that limits the amount of product formed in a chemical reaction. The quantity of.

Mathematics of Chemical Equations By using “mole to mole” conversions and balanced equations, we can calculate the exact amounts of substances that will.

Laboratory 08 LIMITING REACTANT LAB.

Ch. 9 Notes – Chemical Quantities

Percent Yield and Limiting Reactants

Limiting Reactants and Percent Yields

Limiting Reactants & Percent Yield

Starter S moles NaC 2 H 3 O 2 are used in a reaction. How many grams is that?

Ch. 9 Notes -- Stoichiometry

Chapter 9 – Review Stoichiometry

Limiting Reagent and Percent Yield

Limiting and Excess Reagents

Limiting Reagents and Percent Yield

Lecture 109/21/05. Mass reactant Stoichiometric factor Moles reactant Moles product Mass product Stoichiometric Calculations.

Ch. 9: Calculations from Chemical Equations

Stoichiopardy Holy Moley Do the 2 or 3 step Random Limit my Percent Q $100 Q $200 Q $300 Q $400 Q $500 Q $100 Q $200 Q $300 Q $400 Q $500 Final Chempardy.

April 3, 2014 Stoichiometry. Stoichiometry is the study of quantities of materials consumed and produced in chemical reactions Stoikheion (Greek, “element”)

11-3 Limiting Reactants Reactions to this point have had one ingredient in excess. When you are given two or both reactant amounts, you have a limiting.

Chapter 10 Stoichiometry Or One plus One isn’t always Two.

Stoichiometry Kelley Kuhn CCA. What the heck is stoichiometry? Stoichiometry is what we use in chemistry to solve problems. For example, you can use stoichiometry.

STOICHIOMETRY 4 Mole-Mole 4 Mole-Mass 4 Mass-Mass.

Chapter 9 – STOICHIOMETRY The MATH of a CHEMICAL REACTION.

Stoichiometry Ch. 9. The Arithmetic of Equations 9-1.

Limiting Factors & Percent Yield Quiz. Bell Ringer When 6.58 g SO 3 and 1.64 g H 2 O react, what is the expected yield of sulfuric acid? If the actual.

Chapter 12 Stoichiometr y. STOY-KEE-AHM-EH-TREE Founded by Jeremias Richter, a German chemist Greek orgin: stoikheion: element & metron: measure Stoichiometry—the.

Ch. 9 Notes – Chemical Quantities

Stoichiometry Chemical Quantities Chapter 9. What is stoichiometry? stoichiometry- method of determining the amounts of reactants needed to create a certain.

Chapter 12 Stoichiometry. 1. The part of chemistry that deals with the amount of substances involved in chemical reactions A. 3 basic steps to every stoichiometry.

Gravimetric Stoichiometry Is used to calculate masses of reactants and products in a reaction.

The number of bicycles that can be assembled is limited by whichever part runs out first. In the inventory shown in this figure, wheels are that part.

Limiting Reactions and Percent Yield Calculating by moles or mass ©2011 University of Illinois Board of Trustees

Stoichiometry Warmup I have 1 mole of CO 2 gas at STP. How many grams of CO 2 do I have? How many Liters of CO 2 do I have? How many molecules of CO 2.

Ch. 9 Notes – Chemical Quantities Stoichiometry refers to the calculations of chemical quantities from __________________ chemical equations. Interpreting.

Limiting Reagents and Percent Yield Limiting Reagent If you are given one dozen loaves of bread, a gallon of mustard and three pieces of salami, how.

Stoichiometry & Limiting Reactants. Stoichiometric Calculations The coefficients in the balanced equation give the ratio of moles of reactants and products.

Ch. 9 Notes -- Stoichiometry Stoichiometry refers to the calculations of chemical quantities from __________________ chemical equations. Interpreting Everyday.

Ch. 12 Stoichiometry 12.1 The Arithmetic of Equations.

Percent Yield. Definitions The theoretical yield is the maximum amount of product that could be made from the reactants. The actual yield is the amount.

STOICHIOMETRY. What is stoichiometry? Stoichiometry is the quantitative study of reactants and products in a chemical reaction.

Chapter 12: Stoichiometry WASILLLA HIGH SCHOOL

GOOD AFTERNOON! Prepare to take notes. You will be allowed to use these notes on the test next week! You will need: 1.Something to write on 2.Something.

Welcome: 3/10/14 Answer the following question: CaCO 3  CaO + CO 2 How many grams of CO 2 can be made from g of CaCO 3 ?

Ch. 9-3 Limiting Reactants & Percent Yield. POINT > Define limiting reactant POINT > Identify which reactant is limiting in a reaction POINT > Define.

Chemistry Chapter 9 - Stoichiometry South Lake High School Ms. Sanders.

Mass-Mass Conversions 56.0 g N 2 x g N 2 g NH = 1904 = When nitrogen and hydrogen react, they form ammonia gas, which has the formula.

7/6/20161 Chap 9: Stoichiometry 7/6/20162 Section 9-1 Introduction to Stoichiometry Define stoichiometry. Describe the importance of the mole ratio in.

Let’s talk… mole to mole

Stoichiometry and the Mole

Chapter 9: Stoichiometry

Ch. 9 Notes -- Stoichiometry

Chapter 9 STOICHIOMETRY

How much can I make? Maximizing Chemical Quantities

Chapter 12 Review.

Chapter 12 Review.

Mathematics of Chemical Equations

Ch. 9 Notes -- Stoichiometry

Stoichiometry Chapter 12.

Honors Chem Unit 12 Stoich Notes

Limiting Reagent and Percent Yield

Stoichiometry & Limiting Reactants

Chemical Reactions Limiting Reagent.

Chem 111 Ch 9 Notes 9.1 Stoichiometry- calculation of quantities in chemical reactions From the coefficients in a BALANCED equation you can get: N2+3H2

Presentation transcript:

SOL Review 6 Stoichiometry

Consider: 4NH 3 + 5O 2  6H 2 O + 4NO Many conversion factors exist: 4 NH 3 6 H 2 04NO 5O 2 (and others) 5 O 2 4 NO4 NH 3 6 H 2 0 The Coefficients of a balanced chemical reaction can be used to write conversion factors called MOLE RATIOS. With these ratios, you can relate moles of reactants to moles of product.

Consider: 4NH 3 + 5O 2  6H 2 O + 4NO How many moles of H 2 O are produced if mol of O 2 are used? mol H 2 O 6 mol H 2 O 5 mol O 2 x # mol H 2 O=0.176 mol O 2 = Notice that a correctly balanced equation is essential to get the right answer!

Consider: 4NH 3 + 5O 2  6H 2 O + 4NO How many grams of NO are produced if we start with 2.0 moles of O 2 ? We find out how many moles of NO, then convert moles of NO to grams of NO. 2 moles O 2 x 4 moles NO x 30.0 g = 48 g NO 5 moles O 2 1 mole NO

Conversions To Different Units Of Measurement We can also go from liters of a reactant to moles of a product 4NH 3 + 5O 2  6H 2 O + 4NO 4NH 3 + 5O 2  6H 2 O + 4NO How many moles of NO are produced if we start with 3.00 liters of O 2 ? 3 L O 2 x 1 mole x 4 mol NO =.107 mole NO 22.4L 5 mol O L 5 mol O 2

Limiting Reagent: The reactant that limits the amount of the product that can be formed in the reaction. This is the reactant that is completely used up in a reaction. Excess Reagent – reactant that is not completely used up.

Percent yield Percent yield is method for comparing the amount of product made in the lab to the expected result. Reasons why the experimental yield is not the same as the theoretical yield: Not all reactions go to completion. Some may have a “side” reaction and not produce the desired result. Sometimes it is hard to purify the product.

Percent yield = __Actual yield x 100% Theoretical yield The actual yield is the amount made in the lab. The theoretical yield is how much should have been made according to a mass-mass problem using a balanced equation (stoichiometry calculation).

CaCO 3  CaO + CO 2 1. What is the theoretical yield of CaO if 24.8g CaCO 3 is heated? MM CaO = 56 g/mol, MM CaCO 3 = 100 g/mol 24.8 g CaCO 3 x 1 mol CaCO 3 x _1 mol CaO x ___56 g = 100 g 1 mol CaCO 3 1 mol CaO 13.9 g CaO 2. What is the percent yield if 13.1 g is actually produced? 13.1 g x 100% = 94.2% yield 13.9 g